A compound was found to be composed of the following amounts of elements: 20.00% wt% C, 26.64wt% O, 46.65 wt%N, and 6.71wt%H. A 6.125 grams sample of this compound dissolved in 46.205 grams of water as a solution was found to have a freezing point of -3.260C. The density of this solution was 1.066g/mL. Given that the freezing point depression constant and boiling point elevation constan for water are 1.766C/m and .512C/m, respectively answer the following questions.
a) calculate the molality (m) of this solution if the solute is a nonelectrolyte (i=1)
b) calculate of molarity (M) of this solution
c) the boiling point of the above solution
d) calculate the molecular mass of the dissolved solute
e) determine the empirical and molecular formula of the solute